1. Acid-Base Theories

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3. Arrhenius Acids and Bases
Acid produces hydrogen ions (H ) in solution
Base produces hydroxide ions (OH ) in solution
HA ---> H+ + A¯
XOH ---> X+ + OH¯

4. Arrhenius Examples NaOH  OH-(aq) + Na+(aq)
HCl (g)  H+ (aq) + Cl- (aq)
HSO4− → H+(aq) + SO42−(aq)
Ba(OH)2  2OH-(aq) + Ba2+(aq)

5. Neutralization Reactions Classified by Arrhenius!
We get water and salt in a neutralization reaction

6. Bronsted-Lowry Acids and Bases
An acid is a hydrogen ion (H ) donor
A base is a hydrogen ion (H ) acceptor
NH3(aq) + HC2H3O2(aq)  NH4+(aq) + C2H3O2-(aq)
B/L base B/L acid
H2O(l) + HC2H3O2(aq)  H3O+(aq) + C2H3O2-(aq)
B/L base B/L acid
NH3(aq) + H2O(l)  NH4+(aq) + OH-(aq)
B/L base B/L acid

7. Bronsted-Lowry Examples
HCl + H2O  H3O+ + Cl- H2SO4 + H2O  H3O+ + HSO4- HCl + OH-  H2O + Cl-

8. Lewis Acids and Bases An acid is an electron pair acceptor
A + :B → A—B
A base is an electron pair donor
Once you say that an acid is an electron pair acceptor, then you're not limited to the idea that an acid has to be a hydrogen ion or some chemical that contains or releases hydrogen ions. It could be something else, as long as it can accept (or bond to) a pair of electrons.

9. Lewis Examples
H+ + :NH3 → NH4+

10. Properties of an Acid Tastes Sour Conduct Electricity
Corrosive, which means they break down certain substances. Many acids can corrode fabric, skin,and paper
Some acids react strongly with metals
Turns blue litmus paper red
Picture from BBC Revision Bites

11. Uses of Acids Acetic Acid = Vinegar
Citric Acid = lemons, limes, & oranges. It is in many sour candies such as lemonhead & sour patch.
Ascorbic acid = Vitamin C which your body needs to function.
Sulfuric acid is used in the production of fertilizers, steel, paints, and plastics.
Car batteries

12. Properties of a Base Feel Slippery Taste Bitter Corrosive
Can conduct electricity. (Think alkaline batteries.)
Do not react with metals.
Turns red litmus paper blue.

13. Uses of Bases
Bases give soaps, ammonia, and many other cleaning products some of their useful properties.
The OH- ions interact strongly with certain substances, such as dirt and grease.
Chalk and oven cleaner are examples of familiar products that contain bases.
Your blood is a basic solution.

14. pH Scale pH is a measure of how acidic or basic a solution is.
The pH scale ranges from 0 to 14.
Acidic solutions have pH values below 7
A solution with a pH of 0 is very acidic.
A solution with a pH of 7 is neutral.
Pure water has a pH of 7.
Basic solutions have pH values above 7.

15. pH Scale
A change of 1 pH unit represents a tenfold change in the acidity of the solution.
For example, if one solution has a pH of 1 and a second solution has a pH of 2, the first solution is not twice as acidic as the second—it is ten times more acidic.

16. How can we identify strong acids or bases? Easy, memorize them!
Strong Acids and Bases
How can we identify strong acids or bases? Easy, memorize them!
Memorized Strong Acids
HClO4
H2SO4 HI
HBr
HCl
HNO3
Memorized Strong Bases
Hydroxides of group 1 and 2
metals, excluding Be and Mg

17. Acid – Base Reactions
A reaction between an acid and a base is called neutralization. An acid-base mixture is not as acidic or basic as the individual starting solutions.

18. Acid – Base reactions
Each salt listed in this table can be formed by the reaction between an acid and a base.

19. Monoprotic and Polyprotic Acids
Monoprotic can donate one hydrogen ion
HCl + H2O → H3O+ + Cl−
Diprotic can donate two hydrogen ions
H2SO4
Polyprotic is a general term for any acid that can donate more than one hydrogen ion

20. Examples of polyprotic acids
Example: phosphoric acid H3PO4(s) + H2O(l)  H3O+(aq) + H2PO4−(aq) H2PO4−(aq)+ H2O(l)  H3O+(aq) + HPO42−(aq) HPO42−(aq)+ H2O(l)  H3O+(aq) + PO43−(aq)